You have 5 mL of vinegar in a flask and 2 drops of phenolphthalein indicator. You...

You have 5 mL of vinegar in a flask and 2 drops of phenolphthalein indicator. You titrate exactly 36.9 mL of 0.1 mol/L NaOH from a burette directly into the flask which gives you a pale pink color. This means the solution has reached neutralization. Calculate n of the NaOH.

Suppose 0.22 L of 0.5 mol/L NaOH solution was titrated with 5 L of HCl using phenolphthalein indicator. Calculate the amount of the base and the acid that were used to reach the neutralization point.

50 L of 2.0 mol/L Hydrochloric acid is titrated with sodium hydroxide to form water and sodium chloride. How many moles of sodium hydroxide are consumed in this reaction?

You have 5 mL of vinegar in a flask and 2 drops of phenolphthalein indicator. You titrate exactly 36.9 mL of 0.1 mol/L NaOH from a burette directly into the flask which gives you a pale pink color. This means the solution has reached neutralization. Calculate C of the vinegar in mol/L.

00 L of 5 mol/L NaOH are required to fully titrate a 50 L solution of HCl. What is the initial concentration of the acid?

Expert Solution

In the last part the volume of NaOH required is given zero hence the initial concentration of the acid must be zero. we can find this also in a similar way what we did in "d" part.

Amanda K answered 1 year ago

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